For irreversible expansion of an ideal gas under isothermal condition, the correct option is:

At standard conditions, if the change in the enthalpy for the following reaction is $-109 {\mathrm{kJmol}}^{-1}$

${\mathrm{H}}_{2\left(\mathrm{g}\right)}+{\mathrm{Br}}_{2\left(\mathrm{g}\right)}\to 2{\mathrm{HBr}}_{\left(\mathrm{g}\right)}$

Given that bond energy of ${\mathrm{H}}_2$ and ${\mathrm{Br}}_2$ is $435 {\mathrm{kJmol}}^{-1}$ and $192 {\mathrm{kJmol}}^{-1}$, respectively, what is the bond energy (in $\mathrm{kJ} {\mathrm{mol}}^{-1}$) of $\mathrm{HBr}?$

Under the isothermal condition, a gas at $300\mathrm{ }\mathrm{K}$ expands from $0.1\mathrm{ }\mathrm{L}$ to $0.25\mathrm{ }\mathrm{L}$ against a constant external pressure of $2$ bar. The work done by the gas is

(Given that $1\mathrm{ }\mathrm{L}$ bar$=100\mathrm{ }\mathrm{J}$)